(a)
Interpretation:
The aqueous solution of potassium oxalate salt is neutral pH or greater than 7 or less than 7 has to be determined.
Aqueous solution of salt:
The salt is added in water, it will dissolved and generate
Neutral solution:
For the neutral solution, the pH is at 7. In periodic table, group 1 and 2 elements and from other groups those who have +1 charge cations are weak Lewis acids, these hydrated ions does not affect the protons from water. As well as these metal cations are very big, otherwise they may have very small charge to hydrating water molecules to get appreciable polarization effect. These types of cations are called neutral cations because they may not affect the pH of the solution.
The anions from strong acids like halides (except F), nitrates, perchlorates are such weak Lewis bases, so they may not affect the pH of the solution. These anions are called neutral in water.
Acidic solution:
The conjugate acids of weak bases cations make the solution acidic in aqueous medium, because it acts as proton donors. In another case, the metal cations with high charge can act as Lewis acids in aqueous medium solution, even though the cations do not have protons to donate.
Basic solution:
The conjugate bases of weak acids anions make the solution basic in aqueous medium, here, the protons leaves from the negatively charged anions.
(b)
Interpretation:
The aqueous solution of calcium nitrate salt is neutral pH or greater than 7 or less than 7 has to be determined.
Concept introduction:
Refer to part (a).
(c)
Interpretation:
The aqueous solution of methylammonium hydrochloride salt is neutral pH or greater than 7 or less than 7 has to be determined.
Concept introduction:
Refer to part (a).
(d)
Interpretation:
The aqueous solution of potassium phosphate salt is neutral pH or greater than 7 or less than 7 has to be determined.
Concept introduction:
Refer to part (a).
(e)
Interpretation:
The aqueous solution of ferric chloride salt is neutral pH or greater than 7 or less than 7 has to be determined.
Concept introduction:
Refer to part (a).
(f)
Interpretation:
The aqueous solution of pyridinium chloride salt is neutral pH or greater than 7 or less than 7 has to be determined.
Concept introduction:
Refer to part (a).
Want to see the full answer?
Check out a sample textbook solutionChapter 6 Solutions
ACHIEVE/CHEMICAL PRINCIPLES ACCESS 2TERM
- Write the chemical equation and the expression for the equilibrium constant, and calculate Kb for the reaction of each of the following ions as a base. (a) sulfate ion (b) citrate ionarrow_forwardPhosphate ions are abundant in cells, both as the ions themselves and as important substituents on organic molecules. Most importantly, the pKa for the H2PO4 ion is 7.20, which is very close to the normal pH in the body. H2PO4(aq) + H2O() H3O+(aq) + HPO42(aq) 1. What should the ratio [HPO42]/[H2PO4] be to control the pH at 7.40?arrow_forwardThe hydrogen phthalate ion, C8HsO4, is a weak acid with Ka = 3.91 106. C8H5O4(aq)+H2O(l)C8H4O42(aq)+H3O+(aq) What is the pH of a 0.050 M solution of potassium hydrogen phthalate. KC8H5O4? Note: To find the pH for a solution of the anion, we must take into account that the ion is amphiprotic. It can be shown that, for most cases of amphiprotic ions, the H3O+ concentration is [H3O+]=Ka1Ka2 For phthalic acid, C8H6O4 is Ka1 is 1.12 103, and Ka2 is 3.91 106.arrow_forward
- The simplest amino acid is glycine, H2NCH2CO2H. The common feature of amino acids is that they contain the functional groups: an amine group, -NH2, and a carboxylic acid group, -CO2H. An amino acid can function as either an acid or a base. For glycine, the acid strength of the carboxyl group is about the same as that of acetic acid. CH3CO2H, and the base strength of the amino group is slightly greater than that of ammonia, NH3. (a) Write the Lewis structures of the ions that form when glycine is dissolved in 1 M HCl and in 1 M KOH. (b) Write the Lewis structure of glycine when this amino acid is dissolved in water. (Hint: Consider the relative base strengths of the -NH2 and -CO2- groups.)arrow_forwardFor conjugate acidbase pairs, how are Ka and Kb related? Consider the reaction of acetic acid in water CH3CO2H(aq)+H2O(l)CH3CO2(aq)+H3O+(aq) where Ka = 1.8 105 a. Which two bases are competing for the proton? b. Which is the stronger base? c. In light of your answer to part b. why do we classify the acetate ion (CH3CO2) as a weak base? Use an appropriate reaction to justify your answer. In general, as base strength increases, conjugate acid strength decreases. Explain why the conjugate acid of the weak base NH3 is a weak acid. To summarize, the conjugate base of a weak acid is a weak base and the conjugate acid of a weak base is a weak acid (weak gives you weak). Assuming Ka for a monoprotic strong acid is 1 106, calculate Kb for the conjugate base of this strong acid. Why do conjugate bases of strong acids have no basic properties in water? List the conjugate bases of the six common strong acids. To tie it all together, some instructors have students think of Li+, K+, Rb+, Cs+, Ca2+, Sr2+, and Ba2+ as the conjugate acids of the strong bases LiOH, KOH. RbOH, CsOH, Ca(OH)2, Sr(OH)2, and Ba(OH)2. Although not technically correct, the conjugate acid strength of these cations is similar to the conjugate base strength of the strong acids. That is, these cations have no acidic properties in water; similarly, the conjugate bases of strong acids have no basic properties (strong gives you worthless). Fill in the blanks with the correct response. The conjugate base of a weak acid is a_____base. The conjugate acid of a weak base is a_____acid. The conjugate base of a strong acid is a_____base. The conjugate acid of a strong base is a_____ acid. (Hint: Weak gives you weak and strong gives you worthless.)arrow_forward8. (a) HA(aq) is a weak acid with a dissociation constant, Ka, of 8.8 x 10−12. What is the pH of a 0.022 M solution of A−(aq)? The temperature is 25 ◦C. (b) For the reaction A(g) =A(l), the equilibrium constant is 0.666 at 25.0 ◦C and 0.222 at 75.0 ◦C. Making the approximation that the entropy and enthalpy changes of this reaction do not change with temperature, at what temperature will the equilibrium constant be equal to 0.777?arrow_forward
- 3. A 0.0560 g quantity of acetic acid is dissolved in enough water to make 50.0 mL of solution. Calculate the concentrations of H;O*, CH;COO and CH;COOH at equilibrium. What is the pH of the solution? (Ka = 1.8x10) CH;COOH(aq) = CH;COO (aq) + H;O* (aq) a) Calculate the initial concentration of CH;COOH. (C:12; H:1; 0:16) b) Calculate the concentration of CH;CoO (aq) and H;O* (aq) at equilibrium. c) Calculate pH of the solution.arrow_forwardPropionic acid, HC3H5O2, has Ka= 1.34 x 10–5. (a) What is the molar concentration of H3O+ in 0.15 M HC3H5O2 and the pH of the solution? (b) What is the Kb value for the propionate ion, C3H5O2–? (c) Calculate the pH of 0.15 M solution of sodium propionate, NaC3H5O2. (d) Calculate the pH of solution that contains 0.12 M HC3H5O2 and 0.25 M NaC3H5O2.arrow_forwardThe active ingredient of bleach such as Clorox is sodium hypochlorite (NaClO). Its conjugate acid, hypochlorous acid (HClO), has a Ka of 3.0 × 10–8. (a)The undiluted bleach contains roughly 1 M NaClO. Calculate the pH of 1 M NaClO solution. (b)Some applications require extremely diluted bleach solution, such as swimming pools. Suppose the solution in (a) is diluted by 10,000 -fold. Calculate the pH of the diluted solution, and demonstrate that you can still neglect the autoionization of water in your calculation. (c)Suppose the solution in (a) is diluted by 1million-fold, briefly explain how your approach will be different. Write the equation with [H3O+] as the unknown, but you do not need to solve it.arrow_forward
- Determine whether aqueous solutions of the following salts have a pH equal to, greater than, or less than 7; if pH > 7 or pH< 7, write a chemical equation to justify your answer. (a) NH4Br. (b) Na2CO3, (c) KF, (d) KBr, (e) AICI3, (f) Co(NO3)2.arrow_forwardA 0.018 M solution of salicylic acid, HOC6H4CO2H, has the same pH as 0.0038 M HNO3solution. (a) Write an equation for the ionization of salicylic acid in aqueous solution. (Assume only the –CO2H portion of the molecule ionizes.) (b) What is the pH of solution containing 0.018 M salicylic acid? (c) Calculate the Ka of salicylic acid.arrow_forwardCalculate the pH of a solution prepared by dissolving 0.482 mol of benzoic acid and 0.104 mol of sodium benzoate in water sufficient to yield 1.00 L of solution. The K, of benzoic acid is 6.30 x 105. CHSCOOH(aq) + H2O(1) = H3O*(aq) + C6H5CO2 (aq) K = 6.30 × 10-5 A pH = pK, + log; [HA] [* ] %3Darrow_forward
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
- Chemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStax